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Sep 29, 2014 · If we take that one valence electron away, it makes sense to say that it now has zero valence electrons because "1 - 1 = 0". Add a comment. You are correct in that it has 8 valence electrons, not 0. If we look at the electron configuration of potassium (K), we see that it has one electron: [Ar]4s. Obviously, removing that electron gives us [Ar ...
Apr 30, 2017 · At the same time, the Na+/K+ ATPases bring in K+. In summary it is important to note, there is uneven distribution of ions in and outside the cytosol. Because the plasma membrane has more K+ leak channels than Na+ leak channels, the number of K+ ions that leave the cell is greater than the number of Na+ ions that enter the cell.
Cl had a really high ionization energy compared to K and the decrement of the ionization wouldn't be that big to make it less than the ionization energy of KX+. (The answer was that KX+ has more ionization energy than ClX− in the exam paper but I questioning that) So if there is a chart or something for this that would be awesome.
Aug 19, 2018 · Think of it this way: 1) Count the electrons (all of them) in each atom or ion. 2) What happens to the orbitals, and thus to atoms or ions with a given number of electrons (let us say, 18 electrons), when you increase the atomic number of the element (more protons in the nucleus)? Not the answer you're looking for?
Between the species $\ce{Ne, Na+, Mg^2+, Ar, K+, $\&$~Ca^2+}$, which one has the highest ionization energy? I thought that ionization energy increased from left to right in a period and from down to up in a group in the periodic table, so I thought that $\ce{Ne}$ would be the one with the highest ionization energy.
Mar 20, 2018 · According to Wikipedia, the ionic radii of $\ce{ K+}$ is much larger than $\ce{Cu+}$, which makes sense because d-electrons are poor shielders. Also, $\ce{Cu+}$ has larger electron density but it has a higher effective nuclear charge in comparison to potassium ion because of the poor shielding ability of d-electrons.
Oct 30, 2015 · One took a platinum wire inserted into an insulated handle and stuck the wire into a solution containing the potassium ion. One then stuck the wire into a Bunsen burner flame. The last step was to look at the flame using a deep red piece of glass. If potassium was present a rather pretty lilac color was detected.
Aug 30, 2019 · Nothing really is easy if you look deeper, and potassium cation is not smaller than fluorine anion (in terms of ionic radii). $\ce{K+}$ with C.N. 4 is comparable in size with $\ce{F-},$ and then the values of ionic radius for higher C.N. skyrocket to 1.64 Å for C.N. 12. $\endgroup$ –
Apr 27, 2017 · $$\ce{K+, Ca^2+, Al^3+, S^2-, Cl-}$$ Now, I know that the radius decreases as the period progresses to the right and increases as we go down on the P.T. So, I get to this:
Oct 13, 2015 · Although $\ce{Na+}$ has ionic radius of 95 pm and an atomic weight of 23, and $\ce{K+}$ has ionic radius of 133 pm and an atomic weight of 39, hydrated $\ce{Na+}$ is larger than hydrated $\ce{K+}$: This is evident from observing that $\ce{Na+}$ moves through a cell membrane with greater difficulty than $\ce{K+}.$
